By the end of this unit, students should be able to:
• understand the difference between periods and groups
• describe the importance of atomic number in determining the number of electrons
• determine the electron configuration of atoms on the periodic table using the 2n2 rule and the trend in periods and groups
• describe the relationship between valence electrons and element properties
• describe what happens to electrons when excited, and the consequential emission of light.
Electron configuration in the periodic table
students to draw the electron configuration of the first 20 elements in a blank periodic table.
Identify patterns in group and period with shell and electron number and valence
Oxford Science 10 resources
• Check your learning, page 73
By the end of this unit, students should be able to:
• identify the common properties of metals in general
• identify the properties of group 1, 2 and transition metals
• relate the properties of Group 1 and 2 metals to their electron configurations.
Experiment 3.3
The reactivity of metals:
Students compare the reactivity of various metals by observing their reaction with hydrochloric acid.
The Elements app
If you are unable to demonstrate the reactions of group 1 and 2 metals, a great way of allowing students to see their properties is to view them in the ‘The Elements in Action’ app. It costs to purchase the app but it is highly worth it if it can be purchased through the school, as kids love it.
By the end of this unit, students should be able to:
• recognise and identify non-metals and metalloids on the periodic table
• identify and explain the properties of the non-metallic groups, halogens and noble gases.
Challenge 3.4
Identifying patterns in the periodic table:
Students summarise the periodic table, labelling key information and highlighting important groups and information.
Additional resources
Crash Course Chemistry: The Periodic Table (A good, if somewhat fast, summary of the metallic and non-metallic groups as well as the history of Mendeleev’s periodic table) https://www.youtube.com/watch?v=0RRVV4Diomg
3.5 Metal cations and
non-metal anions combine
to form ionic compounds
(pages 78–79)
By the end of this unit, students should be able to:
• define what an ionic compound is
• explain ionic compounds using the terminology ‘anion’ and ‘cation’
• state and explain the charge on an ion
• identify and explain the properties of ionic compounds
• define and identify polyatomic ions
• draw the electron transfer between atoms and the resultant ions
• determine the chemical formulae of ionic compounds.
Experiment 3.5
Conductivity of ionic compounds:
Students investigate the electrical conductivity of two ionic compounds as a solid and in aqueous solution.
Skills Lab 3.5
Ionic compounds:
Students apply their understanding of the charges on ions to develop chemical formulas for ionic compounds.
Ionic compounds
Once students have completed the Skills Lab 3.5, as an extension, give them a valency table (there are many on the internet) and get them to create a test which they can give to other students. The test should focus on two sets of questions: 1. How to name ionic compounds from formulae; and 2. How to develop the formulae of ionic compounds from names.
the size of the atom gets smaller going left to right across aperiod
metals get more reactive going down the group
non metals get more reactive as you go up the group
The number at the top of the group can tell you how many electrons in the outer shell
the Period number the element is in can tell you how many shells the atom has.
The valency of an element can be determined (generally) by its group--eg elements in group 1 have a valency of 1 . If they lose an electron they become a positive ion a cation We would write this as a 1 + to the top right of the elements symbol
Eg 2 a metal in group 2 will have a valency of 2 . if they lose 2 electrons they will have a 2+ charge (cation)
Eg a non metal in group 17 will have a valency of 1 they will gain one electron and become a negative ion or anion. We will write it a 1- to the top right of the elements symbol
Some basic properties of metals
they are shiny when cut
they are good conductors of heat
they are good conductors of electricity
they can be beaten into a shape - maleable
they can be drawn into a wire - ductile
they are hard at room temperature - except mercury
they have high boiling points and a range of melting points.
Non Metals
They are brittle or gaseous
they can form covalent bonds with each other
they form ionic binds with metals ( eg sodium chloride)
Calculating the number of protons and neutrons and electrons using the atomic number and the atomic mass
Atomic number is generally the smallest number - = the number of electrons it also equals the number of protons
Mass number is the biggest number - its the combination of the number of protons and the number of neutrons
Eg Mass number of 23 Atomic number 11
this means this atom has 11 protons, 11 electrons
and protons + neutrons = 23
therefore neutrons = 23 -11 = 12 neutrons
Electron Configuration
This is the name of the pattern the electrons form as the orbit the nucleus of an atom.
The electron shells fill up in order
The maximum number of electrons that fit into the first four shell is as follows 2.8.8.18.
Some examples
Hence we write the electron configuration of sodium as 2.8.1
And the electron configuration of chlorine as 2.8.7
and the electron configuration of calcium as 2.8.8.2
And the electron config of copper as 2.8.15.2
and for the calcium cation Ca2+ 2.8.8
Flame test Prac
Theory: when a metal is heated electrons are excited and move to a higher energy level. (this means one or two electrons move out to an outer shell). They continue to orbit there until they slow and eventually return to their original energy level (ground state). As they return to their ground state they release energy in the form of coloured light. Every element has its own special colour.
Name
................Colour
....... safety
Strontium Chloride
Bright red
eye damage in a crystal form
Barium CHloride
White yellow
Toxic if swallowed
Copper Chloride
Green (some blue)
eye damage if crystalline
Potassium Chloride
Light purple/ peachy pink
toxic if swallowed, wash off skin
Sodium Chloride
Orange
eye damage if crystalline
Calcium Chloride
Blood Orange
Toxic
Lithium Chloride
Dark red
harmful if swallowed
Strontium nitrate
orange/red
risk of explosion crystal
Metal Families Prac
How do the metals react?
Metals
.............conducts electricity
......reacts with water
...........reacts with HCl
Cu
y
n
yes slow
Mg
y
n
yes vigorous
Fe
y
y slow
yes slow
CuCl2
as a solid - no
dissolves
dissolves
CaCl2
no as asolid
dissolves
dissolves
Metals vs Compounds
Pure metals have different properties to metals when they are combined with non metals.
Pure metals conduct electricity and react with acids to make hydrogen gas.
Compounds of metals and nonmetals are called salts - they are brittle and do not conduct electricity.
4.3 When atoms meet -- How ionic compounds are made p 177
An atom has a neutral charge - this means the number of protons = the number of electrons.
Remember the protons are positive charges inside the nucleus. They can not be taken out of the nucleus.
The electrons are negative charges and orbit the nucleus. they can be added to or removed.
anions are the negative charged atoms
cations are positive charged atoms
To make a cation we remove electrons form the outer shell. This means the atom has more positive protons than negative electrons and hence an overall positive charge. The way we write this - a Ca atom loses 2 electrons therefore it has 2 more protons than electrons at this point in time. the charge atom is called a cation and is written with a 2+ on the top write of the the elements symbol.
Eg Ca ---------> Ca2+ (+ 2 e)
To make an anion we add electrons to the outer shell. This means there are more negative electrons than positive protons and hence a negative charge.
Eg Cl (+ e) ----------> Cl-
Ionic compounds are formed by combining anions and cations.
This is because the negative ion is attracted to the positive ion and make a strong bond between the atoms.
This bond is called an ionic bond. An example of an ionic compound is sodium chloride (salt).
Writing formula for ionic compounds
The main idea
1. only metals join with non metals ( check your periodic table)
2. The number of electrons in the outer shell determines the valency of an atom
(method: valency = the number of electrons in outer shell if there are less than 4 ( if there is less than 4 electrons its a metal)
valency = 8 - the number of electrons in the outer shell for non metals - (if there are more than 4 electrons in the outer shell its a nonmetal
NB This is a generalisation for the first 24 elements and does not work for elements above atomic number 24.
3. because in an ionic bond the metal atom donates electrons to the nonmetal atom charged atoms are created - a charged atom is an ion.
4. if you can't do 2. above - use this table below here, which tells you the valency
writing the formulae
eg. A solution of Lead Nitrate reacts with a solution of Aluminium Chloride. Solution means in water = (aq)
Big numbers are only used in front of the compound
Little numbers are used inside the compound - they may be behind the metal or the nonmetal
NB little numbers tell you how many of that atom of the element are required to make the compound .. eg H2O the 2 is behind the H therefore there are 2 H atoms in the compound water. There is an imaginary 1 behind the O therefore there is only 1 O atom in a molecule of water
Step 1. Determine the symbol and charge of each ion (the numerals in () represent the ion’s charge) but write the cation (+ ions) before the non-metal anion(s) (- ions) except for substances with acetate.
CATIONS
ANIONS
1+
2+
3+
1-
2-
3-
Ammonium NH4+
Barium Ba2+
Aluminium Al3+
Bicarbonate HCO3-
Carbonate CO32-
Nitride N3-
Cuprous (I) Cu+
Beryllium Be2+
Chromium Cr3+
Bromide Br-
Chromate CrO42-
Phosphate PO43-
Hydrogen H+
Calcium Ca2+
Ferric (III) Fe3+
Chloride Cl-
Dichromate Cr2O72-
Phosphide P3-
Lithium Li+
Copper (II) Cu2+
Chlorate ClO3-
Zincate Zn(OH)42-
Potassium K+
Iron (II) Fe2+
Permanganate MnO4-
Silicate SiO32-
Silver Ag+
Lead (II) Pb2+
Acetate CH3COO-
Oxide O2-
Sodium Na+
Magnesium Mg2+
Fluoride F-
Peroxide O22-
Strontium Sr2+
Hydride H-
Sulfate SO42-
Tin Sn2+
Hydroxide OH-
Sulfide S2-
Zinc Zn2+
Iodide I-
Sulfite SO32-
Mercury Hg2+
Nitrate NO3-
Thiosulfate S2O32-
Nitrite NO2-
Step 2. To write a chemical formula, write ONE of each ion & balance the ion charges so the total is 0 by writing the required coefficient to the bottom right of the ion. For multiples of an atom group, use ( ).
eg. Al3+Cl-, Charge number of Al is a 3 and the charge number of Cl is a 1 so Al1Cl3 but write it as AlCl3
eg. Pb2+NO3- . Charge number on Pb is a 2, and NO3 is only a 1 so Pb1(NO3)2 but write it as Pb(NO3)2.
Chemical Patterns (updated for new text)
Key Concepts
SCIENCE UNDERSTANDING The atomic structure and properties of elements are used to organise them in the periodic table. Elaborations Recognising that elements in the same group of the periodic table have similar properties Describing the structure of atoms in terms of electron shells Explaining how the electronic structure of the atom determines its position in the periodic table and its properties Investigating the chemical activity of metals
NAME:
Timing 8 lessons Assessment: experimental design interpretation. Topic test via assesson.
Science Quest TEXTBOOK
SCIENCE Quest PRACTICALS / ACTIVITIES
SCIENCE Quest HOMEWORK
OTHER ACTIVITIES/RESOURCES
1
Patterns, Order and organisation p 166
Elements in the same group have similar properties. P134 to 138 - Properties, metal, non-metals, atomic number and atomic mass (review from yr9)
Following a trend: Copy table “Patterns in the periodic table” p140
Assesson Pretest
Investigation 4.1 Chem properties of metals and non-metals.
Investigation 4.2 Comparing the properties of 2 metal families
Digital documents: (doc 8470) Revising Chemical patterns (Individual Pathways Activity 4.1 Revising chemical patterns)
Assesson Progress Test
Ques. From textbook – 1 to 5 p 140 or 141 Extension: ( doc 8471) –Investigating chemical patterns Extension: Interactive: __Time Out: 'Periodic Table'__
[ int-0758 ]
Words to Learn Periods, groups, atomic number, relative atomic mass, noble gases, non metals, metals, transition metals, lustre, conductor, insulator, ductile, brittle
2
4.2 Small but important p 142
Describing the structure of atoms in terms of electron shells
Explaining how the electronic structure of the atom determines its position in the periodic table and its properties
Use the concept of electron shells to explain observation from flame tests. (not absorption spectrum)
Assesson Pretest
Interactive: Shell Shocked (int- 0676)
Draw the electron shell diagram for 4 different elements
Investigation 4.3 p 143. Flame Tests
Text book Ques: p144, q2, 3, 6, 7,
Assesson Progress Test
Work Sheets -down load from digital resource in text book 4.3 Electron Shells, 4.4 The structure of an atom
Words to Learn Electron shell, electronic configuration,
3
4.3 When atoms meet p 145
How are anions and cations made
Ionic compounds are formed by combining anions and cations. Define an ionic bond.
Writing ionic formulae
(Do not do covalent bonding)
Assesson Pretest
Summarise p145 to 147
Test book ques p147 q 1 to 5
Use electron dot diagrams to draw an ionic compound
Digital Documents Ionic bonding
Assesson Progress Test
Hmwk p147 q 6 to 8 and q 11 Extension q10 p 147
Digital Documents Writing formula for ionic compounds
4.5 Science as a Human Endeavour: How Reactive p150
Investigating the chemical activity of metals
Describe a replacement reaction
Assesson Pretest
Investigation 4.4 p151 Investigating reactivity of metals
Read p 151 to 152
Copy Activity Series p 151
P152 ques 1
Assesson Progress Test
Ext 3 and 6 – (poster to present results from Investigating reactivity of metals)
ext eLesson Davey and Potassium p151
Words to Learn Mineral ores, displacement reaction, smelting, alloy, bronze,
Investigation; reportable Writing an experimental method Interpreting observations
Watch a video and record the method, interpret the observations
5
4.6 Finding the right formula p153
Valency
Ionic formula (leave out covalent bonding and formula- other than water and carbondioxide and the table for common nonmetals and their molecular formulae
Revision and test
P 153Copy table of common nonmetal molecules and their molecular formulae.
p 153 Copy valency table
p 154 Copy common positive ions and common negative ions.
determines its properties
(pages 70–73)
VCSSU123
Science Inquiry Skills
VCSIS135
VCSIS136
VCSIS137
VCSIS139
VCSIS140
• understand the difference between periods and groups
• describe the importance of atomic number in determining the number of electrons
• determine the electron configuration of atoms on the periodic table using the 2n2 rule and the trend in periods and groups
• describe the relationship between valence electrons and element properties
• describe what happens to electrons when excited, and the consequential emission of light.
Electron configuration in the periodic table
students to draw the electron configuration of the first 20 elements in a blank periodic table.
Identify patterns in group and period with shell and electron number and valence
• Check your learning, page 73
Additional resources
PhET Build and Atom: https://phet.colorado.edu/en/simulation/build-an-atom
table have properties
in common
(pages 74–75)
VCSSU123
Science Inquiry Skills
VCSIS135
VCSIS136
VCSIS139
VCSIS140
• identify the common properties of metals in general
• identify the properties of group 1, 2 and transition metals
• relate the properties of Group 1 and 2 metals to their electron configurations.
The reactivity of metals:
Students compare the reactivity of various metals by observing their reaction with hydrochloric acid.
The Elements app
If you are unable to demonstrate the reactions of group 1 and 2 metals, a great way of allowing students to see their properties is to view them in the ‘The Elements in Action’ app. It costs to purchase the app but it is highly worth it if it can be purchased through the school, as kids love it.
• Check your learning, page 75
• Experiment 3.3, page 195
Brainiac: Reactivity of alkali metals
https://www.youtube.com/watch?v=m55kgyApYrY
(pages 76–77)
VCSSU123
Science Inquiry Skills
VCSIS135
VCSIS139
VCSIS140
• recognise and identify non-metals and metalloids on the periodic table
• identify and explain the properties of the non-metallic groups, halogens and noble gases.
Identifying patterns in the periodic table:
Students summarise the periodic table, labelling key information and highlighting important groups and information.
• Check your learning, page 77
• Challenge 3.4, page 196
Crash Course Chemistry: The Periodic Table (A good, if somewhat fast, summary of the metallic and non-metallic groups as well as the history of Mendeleev’s periodic table)
https://www.youtube.com/watch?v=0RRVV4Diomg
non-metal anions combine
to form ionic compounds
(pages 78–79)
VCSSU123
Science Inquiry Skills
VCSIS135
VCSIS136
VCSIS138
VCSIS139
VCSIS140
• define what an ionic compound is
• explain ionic compounds using the terminology ‘anion’ and ‘cation’
• state and explain the charge on an ion
• identify and explain the properties of ionic compounds
• define and identify polyatomic ions
• draw the electron transfer between atoms and the resultant ions
• determine the chemical formulae of ionic compounds.
Conductivity of ionic compounds:
Students investigate the electrical conductivity of two ionic compounds as a solid and in aqueous solution.
Skills Lab 3.5
Ionic compounds:
Students apply their understanding of the charges on ions to develop chemical formulas for ionic compounds.
Ionic compounds
Once students have completed the Skills Lab 3.5, as an extension, give them a valency table (there are many on the internet) and get them to create a test which they can give to other students. The test should focus on two sets of questions: 1. How to name ionic compounds from formulae; and 2. How to develop the formulae of ionic compounds from names.
• Check your learning, page 79
• Experiment 3.5, page 197
• Skills lab 3.5, page 198
Class notes
where are the following in the periodic table?
Colour these in on your periodic table
Patterns across the periodic table
The valency of an element can be determined (generally) by its group--eg elements in group 1 have a valency of 1 . If they lose an electron they become a positive ion a cation We would write this as a 1 + to the top right of the elements symbol
Eg 2 a metal in group 2 will have a valency of 2 . if they lose 2 electrons they will have a 2+ charge (cation)
Eg a non metal in group 17 will have a valency of 1 they will gain one electron and become a negative ion or anion. We will write it a 1- to the top right of the elements symbol
Some basic properties of metals
Non Metals
They are brittle or gaseous
they can form covalent bonds with each other
they form ionic binds with metals ( eg sodium chloride)
Calculating the number of protons and neutrons and electrons using the atomic number and the atomic mass
Eg Mass number of 23 Atomic number 11
this means this atom has 11 protons, 11 electrons
and protons + neutrons = 23
therefore neutrons = 23 -11 = 12 neutrons
Electron Configuration
Some examples
Flame test Prac
Theory: when a metal is heated electrons are excited and move to a higher energy level. (this means one or two electrons move out to an outer shell). They continue to orbit there until they slow and eventually return to their original energy level (ground state). As they return to their ground state they release energy in the form of coloured light. Every element has its own special colour.
Metal Families Prac
How do the metals react?
Metals vs Compounds
4.3 When atoms meet -- How ionic compounds are made p 177
To make a cation we remove electrons form the outer shell. This means the atom has more positive protons than negative electrons and hence an overall positive charge. The way we write this - a Ca atom loses 2 electrons therefore it has 2 more protons than electrons at this point in time. the charge atom is called a cation and is written with a 2+ on the top write of the the elements symbol.
Eg Ca ---------> Ca2+ (+ 2 e)
To make an anion we add electrons to the outer shell. This means there are more negative electrons than positive protons and hence a negative charge.
Eg Cl (+ e) ----------> Cl-
Ionic compounds are formed by combining anions and cations.
This is because the negative ion is attracted to the positive ion and make a strong bond between the atoms.
This bond is called an ionic bond. An example of an ionic compound is sodium chloride (salt).
Writing formula for ionic compounds
The main idea
1. only metals join with non metals ( check your periodic table)
2. The number of electrons in the outer shell determines the valency of an atom
(method: valency = the number of electrons in outer shell if there are less than 4 ( if there is less than 4 electrons its a metal)
valency = 8 - the number of electrons in the outer shell for non metals - (if there are more than 4 electrons in the outer shell its a nonmetal
NB This is a generalisation for the first 24 elements and does not work for elements above atomic number 24.
3. because in an ionic bond the metal atom donates electrons to the nonmetal atom charged atoms are created - a charged atom is an ion.
4. if you can't do 2. above - use this table below here, which tells you the valency
writing the formulae
eg. A solution of Lead Nitrate reacts with a solution of Aluminium Chloride. Solution means in water = (aq)
Big numbers are only used in front of the compound
Little numbers are used inside the compound - they may be behind the metal or the nonmetal
NB little numbers tell you how many of that atom of the element are required to make the compound .. eg H2O the 2 is behind the H therefore there are 2 H atoms in the compound water. There is an imaginary 1 behind the O therefore there is only 1 O atom in a molecule of water
Step 1. Determine the symbol and charge of each ion (the numerals in () represent the ion’s charge) but write the cation (+ ions) before the non-metal anion(s) (- ions) except for substances with acetate.
Step 2. To write a chemical formula, write ONE of each ion & balance the ion charges so the total is 0 by writing the required coefficient to the bottom right of the ion. For multiples of an atom group, use ( ).
eg. Al3+Cl-, Charge number of Al is a 3 and the charge number of Cl is a 1 so Al1Cl3 but write it as AlCl3
eg. Pb2+NO3- . Charge number on Pb is a 2, and NO3 is only a 1 so Pb1(NO3)2 but write it as Pb(NO3)2.
Chemical Patterns (updated for new text)
The atomic structure and properties of elements are used to organise them in the periodic table.
Elaborations
Recognising that elements in the same group of the periodic table have similar properties
Describing the structure of atoms in terms of electron shells
Explaining how the electronic structure of the atom determines its position in the periodic table and its properties
Investigating the chemical activity of metals
Timing 8 lessons
Assessment: experimental design interpretation.
Topic test via assesson.
TEXTBOOK
HOMEWORK
Extension: ( doc 8471) –Investigating chemical patterns
Extension: Interactive: __Time Out: 'Periodic Table'__
[ int-0758 ]
Periods, groups, atomic number, relative atomic mass, noble gases, non metals, metals, transition metals, lustre, conductor, insulator, ductile, brittle
4.3 Electron Shells,
4.4 The structure of an atom
Electron shell, electronic configuration,
- How are anions and cations made
- Ionic compounds are formed by combining anions and cations. Define an ionic bond.
- Writing ionic formulae
(Do not do covalent bonding)Extension q10 p 147
doc-8641.doc
- __Details__
- __Download__
- 673 KB
- Worksheets from text book -
- 4.5 Ionic bonding
- 4.6 Writing formulae for ionic compounds
- Electron Configuration
2. __. try this simulation on balancing equations__This simulation takes a bout 120 seconds to load and you will need to read the instructions to get the best out of this simulation.Cation, anion, ionic compound,
ext eLesson Davey and Potassium p151
Mineral ores, displacement reaction, smelting, alloy, bronze,
Writing an experimental method
Interpreting observations
Revision and test
Year10 Chemical Pattern